the balanced equation for the above reaction is HBr + KOH ---> KBr + H₂O stoichiometry of HBr to KOH is 1:1 HBr is a strong acid and KOH is a strong base and they both completely dissociate. The number of HBr moles present - 0.25 M / 1000 mL/L x 52.0 mL = 0.013 mol The number of KOH moles added - 0.50 M / 1000 mL/L x 26.0 mL = 0.013 mol the number of H⁺ ions = number of OH⁻ ions therefore complete neutralisation occurs. Therefore solution is neutral. At 25 °C, when the solution is neutral, pH = 7. Then pH of solution is 7
